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Calculate ∆H° for the following reaction:
2H3BO3(aq) → B2O3(s) + 3H2O(l)
a) H3BO3(aq) → HBO2(aq) + H2O(l) , ∆`H_1^@` = − 0.02 kJ
b) H2B4O7(s) → 2B2O3(s) + H2O(l) , ∆`H_2^@` = 17.3 kJ
c)H2B4O7(s) + H2O(l) → 4HBO2(aq), ∆`H_3^@` = − 11.58 kJ
Concept: Chemical Thermodynamics and Energetic >> Enthalpy of Bond Dissociation
What are the conditions for spontaneous and non-spontaneous reactions in terms of free
energy change?
Concept: Chemical Thermodynamics and Energetic >> Free Energy Change for Spontaneous and Non Spontaneous Processes
What is the action of heat on potassium permanganate?
Concept: Chemical Thermodynamics and Energetic >> Work, Heat, Energy, Extensive and Intensive Properties
Derive the equation : W = - PextAV
Concept: Chemical Thermodynamics and Energetic >> Work, Heat, Energy, Extensive and Intensive Properties
The process in which the value of ΔU = 0 is __
Concept: Chemical Thermodynamics and Energetic >> Types of Systems
Give two uses of the Third law of thermodynamics.
Concept: Chemical Thermodynamics and Energetic >> Second and Third Law of Thermodynamics
Calculate the internal energy at 298K for the formation of one mole of ammonia, if the enthalpy change at constant pressure is – 42.0 kJ mol-1.
(Given: R = 8.314 J K-1 mol-1)
Concept: Chemical Thermodynamics and Energetic >> First Law of Thermodynamics
A system absorbs 6 kJ of heat and does 1.5 kJ of work on its surroundings. The change in internal energy is __________.
Concept: Chemical Thermodynamics and Energetic >> Internal Energy and Enthalpy
Write the conditions for maximum work done by the system.
Concept: Chemical Thermodynamics and Energetic >> Chemical Thermodynamics and Energetic
Calculate the work done in the following reaction at 50°C. State whether work is done on the system or by the system.
`"SO"_2("g") + 1/2"O"_(2("g")) rightarrow "SO"_(3("g"))`
Concept: Chemical Thermodynamics and Energetic >> Enthalpy of Bond Dissociation
The standard enthalpy of combustion of formaldehyde Δ0H0 = -571 kJ. How much heat will be evolved in the formation of 22 g of CO2?
Concept: Chemical Thermodynamics and Energetic >> Combustion, Formation, Atomization, Sublimation
5 moles of helium expand isothermally and reversibly from a pressure 40 × 10-5 N m-2 to 4 × 10-5 N m-2 at 300 K. Calculate the work done, change in internal energy and heat absorbed during the expansion. (R = 8.314 J K-1 mol-1).
Concept: Chemical Thermodynamics and Energetic >> Work, Heat, Energy, Extensive and Intensive Properties
Write features of a reversible process.
Concept: Chemical Thermodynamics and Energetic >> Chemical Thermodynamics and Energetic
A substance which shows the highest entropy is ___________.
Concept: Chemical Thermodynamics and Energetic >> Dilution Introduction of Entropy as a State Function
Choose the most correct answer:
Which of the Na following is a buffer solution?
Concept: Buffer Solutions
Choose the most correct answer :
For pH > 7 the hydronium ion concentration would be _________.
Concept: The pH Scale
Answer the following in brief :
What are acids and bases according to Arrhenius theory?
Concept: Acids and Bases in Daily Life
In NaOH solution [OH–] is 2.87 × 10–4. Calculate the pH of the solution.
Concept: The pH Scale
For a reaction \[\ce{HCl_{(aq)} + H2O_{(l)} ⇌ H3O^+_{ (aq)} + Cl^-_{ (aq)}}\]
Which of the following is a conjugate acid-base pair?
Concept: Acids and Bases in Daily Life
The theory which explain amphoteric nature of water is ______.
Concept: Acids and Bases in Daily Life
